Rates and the idea of excess or limiting factor

Question 1

Explain the method

Answer 1

They used a balance to measure out 2.00g of calcium carbonate lumps which were
placed in the conical flask.
They also added 50.0cm3 of 0.250 moldm-3 nitric acid to the conical flask before replacing the bung and using the gas syringe to measure the volume of gas produced

Question 2

Write the equation for the reaction between calcium carbonate and nitric acid

Answer 2

CaCO3 (aq) + 2HNO3(aq) → Ca(NO3)2(aq) + CO2(g) + H2O(l)

Question 3

What would increasing the mass of calcium carbonate do to the rate of reaction?

Answer 3

Increase rate of reaction

Question 4

What would increasing the volume of gas produced do to the rate of reaction?

Answer 4

Stay the same

Question 5

What would using 50cm3 of 0.500 mol dm-3 nitric acid rather than 0.250 mol dm-3 of nitric acid do to the rate of reaction

Answer 5

Increase rate of reaction

Question 6

What would increasing the volume of gas produced do to the rate of reaction?

Answer 6

Increase rate of reaction

Question 7

What would using the same mass of powdered CaCO3 rather than lumps do to the rate of reaction?

Answer 7

Increase rate of reaction

Question 8

What would increasing the volume of gas produced do to the rate of reaction?

Answer 8

Stay the same